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can sum1 explain me the shielding effect of inner electrons?
Shielding effect plays a role in ionisation energies and therefore in reactivity. Shielding usually decreases the effective nuclear force, which makes the outermost electrons experience less of an attraction meaning the electron can be removed with more ease. Shielding effect increases as you go down the group as you have increasing number of energy levels, whereas going across the period, shielding effects usually remain rather constant.
In exam questions they usually ask for a general trend, e.g. Why is there a general increase in the first ionisation energy as you go across the period? or they ask you to compare e.g. Why is the first ionisation energy of phosphorus greater than that of sulfur? or Why is the first ionisation energy of of magnesium greater than that of aluminium?
When answering those questions you should include: distance from the nucleus, effective nuclear charge (causes the atomic radius to decrease, meaning ionisation energies are higher since the electrons are nearer to the nucleus) , increasing nuclear charge, shielding effects and interelectronic repulsion (from paired electrons).
If you know the answers to those questions you should be ok for that section.
Hope it helps.